A chemical reaction by definition forms new chemicals (called the products) from the initial chemicals (called the reactants). It should make sense that the identity of the products formed depends on what reactants we start with. Adding an acid to a base is an example of a chemical reaction, so we should expect to see new products. Although there is a pattern to this type of reaction, ultimately the products formed depend on what acid and what base are used.
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mechanical
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They have a crystalline structure.
B.
They contain useful metals.
C.
They are made of silicon and oxygen.
D.
They are too hard to be scratched with a nail.
b. A 100.0 g sample of liquid ethanol vaporizes at its boiling point. Hvap = 38.6 kJ/mol
The heat required for the following two processes are:
a. 10.74 KJ
b. 83.92 KJ
Part a)
Given:
Mass (m) of ethanol = 100g
Heat of fusion, Hfus = 4.94 kJ/mol
To find:
Heat (Q) =?
Mass of C₂H₅OH = 100g
Molar mass of C₂H₅OH = (2x12)+ (5x1) + 16 + 1 = 46g/mol
Number of Mole = Mass /Molar Mass
Number of mole (n) of C₂H₅OH = 100/46 = 2.174 moles.
Calculation for Heat of fusion:
Q = n x Hfus
Q = 2.174 mol x 4.94 kJ/mol
Q = 10.74KJ
Therefore, 10.74 KJ of heat is required to melt the ethanol.
Part b)
Given:
Mass of C₂H₅OH = 100g
Heat of vaporization, Hvap = 38.6 kJ/mol
To find:
Heat (Q) =?
Calculation for Heat of vaporization:
As calculated above, the number of mole in 100g of ethanol, C₂H₅OH is 2.174 moles.
The heat required to vaporize the ethanol can be obtained as follow:
Q = n x Hvap
Q = 2.174 mol x 38.6 kJ/mol
Q = 83.92 KJ
Therefore, 83.92 KJ of heat is required to vaporize the ethanol.
Find more information about Heat of fusion here:
Answer:
A. 10.74 KJ
B. 83.92 KJ
Explanation:
A. Data obtained from the question include the following:
Mass (m) of ethanol = 100g
Heat of fusion, Hfus = 4.94 kJ/mol
Heat (Q) =..?
Next, we shall determine the number of mole in 100g of ethanol, C2H5OH. This is illustrated below:
Mass of C2H5OH = 100g
Molar mass of C2H5OH = (2x12)+ (5x1) + 16 + 1 = 46g/mol
Number of mole (n) of C2H5OH =..?
Mole = Mass /Molar Mass
Number of mole (n) of C2H5OH = 100/46 = 2.174 moles.
Now, we can obtain the heat required to melt the ethanol as follow:
Q = n x Hfus
Q = 2.174 mol x 4.94 kJ/mol
Q = 10.74KJ
Therefore, 10.74 KJ of heat is required to melt the ethanol.
B. Data obtained from the question include the following:
Mass of C2H5OH = 100g
Heat of vaporisation, Hvap = 38.6 kJ/mol
Heat (Q) =..?
As calculated above, the number of mole in 100g of ethanol, C2H5OH is 2.174 moles.
The heat required to vaporise the ethanol can be obtained as follow:
Q = n x Hvap
Q = 2.174 mol x 38.6 kJ/mol
Q = 83.92 KJ
Therefore, 83.92 KJ of heat is required to vaporise the ethanol.
C. From the above calculations, a higher amount of heat energy i.e 83.92 KJ is required to vaporise the ethanol and a lesser amount of heat energy i.e 10.74 KJ is needed to melt the ethanol.
(b) by sharing electrons with each other
(c) by losing neutrons to each other
(d) by losing electrons
Answer:
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Explanation: